Concept explainers
(a)
Interpretation:
Nature of the bond is whether nonpolar covalent or polar covalent or ions has to classified.
Concept introduction:
Nature of the bond:
Nature of the bond is based on the electronegativity difference between the bonded atoms.
Non polar covalent bond is formed when the electronegativity difference between the bonded atoms is less than 0.5.
Polar covalent bond is formed when the electronegativity difference between the bonded atoms is 0.5 to 1.9.
The ions formed when the electronegativity difference between the bonded atoms is more than 1.9.
(b)
Interpretation:
Nature of the bond is whether nonpolar covalent or polar covalent or ions has to classified.
Concept introduction:
Nature of the bond:
Nature of the bond is based on the electronegativity difference between the bonded atoms.
Non polar covalent bond is formed when the electronegativity difference between the bonded atoms is less than 0.5.
Polar covalent bond is formed when the electronegativity difference between the bonded atoms is 0.5 to 1.9.
The ions formed when the electronegativity difference between the bonded atoms is more than 1.9.
(c)
Interpretation:
Nature of the bond is whether nonpolar covalent or polar covalent or ions has to classified.
Concept introduction:
Nature of the bond:
Nature of the bond is based on the electronegativity difference between the bonded atoms.
Non polar covalent bond is formed when the electronegativity difference between the bonded atoms is less than 0.5.
Polar covalent bond is formed when the electronegativity difference between the bonded atoms is 0.5 to 1.9.
The ions formed when the electronegativity difference between the bonded atoms is more than 1.9.
(d)
Interpretation:
Nature of the bond is whether nonpolar covalent or polar covalent or ions has to classified.
Concept introduction:
Nature of the bond:
Nature of the bond is based on the electronegativity difference between the bonded atoms.
Non polar covalent bond is formed when the electronegativity difference between the bonded atoms is less than 0.5.
Polar covalent bond is formed when the electronegativity difference between the bonded atoms is 0.5 to 1.9.
The ions formed when the electronegativity difference between the bonded atoms is more than 1.9.
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Chapter 1 Solutions
Organic Chemistry
- Identify the electron pair geometry, the molecular structure of each, and the polarity of the following molecules: (a) ClNO (N is the central atom) (b) Cl2CO (C is the central atom) (c) Cl2SO (S is the central atom) (d) SO2F2 (S is the central atom) (e) XeO2F2 (Xe is the central atom) (f) ClOF2 + (Cl is the central atom)arrow_forwardWrite the Lewis structures for the following, and include resonance structures where appropriate. Indicate which has the strongest carbon-oxygen bond.(a) CO2(b) COarrow_forwardii. Answer true or false. (a) A covalent bond is formed between two atoms whose difference in electronegativity is less than 1.9. (b) If the difference in electronegativity between two atoms is zero (they have identical electronegativities), then the two atoms will not form a covalent bond. (c) A covalent bond formed by sharing two electrons is called a double bond. (d) In the hydrogen molecule (H2), the shared pair of electrons completes the valence shell of each hydrogen. (e) In the molecule CH4, each hydrogen has an electron configuration like that of helium, and carbon has an electron configuration like that of neon. (f) In a polar covalent bond, the more electronegative atom has a partial negative charge (8-) and the less electronegative atom has a partial positive charge (&+). (g) These bonds are arranged in order of increasing polarity C-Harrow_forwardConsider the collection of nonmetallic elements O, P, Te,I, and B. (a) Which two would form the most polar singlebond? (b) Which two would form the longest single bond?(c) Which two would be likely to form a compound of formulaXY2? (d) Which combinations of elements would likelyyield a compound of empirical formula X2Y3?arrow_forwardIn each case, tell whether the bond is ionic, polar cova- lent, or nonpolar covalent. (a) Br, (e) SiH, (d) SrF, (c) HCl (g) N, (b) BrCl 2 (f) CO (h) CsCl 4.arrow_forwardDraw Lewis diagrams for the following ions. In the formula the symbol of the central atom is given first. (Hint:The valence octet may be expanded for the central atom.)(a) BrO4 - (b) PCl6 - (c) XeF6+arrow_forwardWhich of the following is a resonance structure of compound X? N (A) OH NH (B) X NH O NH (C) N (D)arrow_forwardWrite Lewis dot symbols for the following atoms and ions. (a) I (b) I− (c) S (d) S2−arrow_forwardAn elemental analysis of a hydrocarbon, which contains only carbon and hydrogen, shows the mass%: element mass% carbon 92.26 hydrogen 7.743 (A) * Determine the empirical formula of the hydrocarbon. (B) The compound has a molar mass of 26.04 g/mol. Determine its molecular formula. (C, Draw the Lewis structure of the molecular compound. Count the total number of sigma bonds and pi bonds each, present in the molecule. (D, What is the hybridization of carbon in the molecule? Explain.arrow_forwardDraw Lewis structures for the following compounds. Remember to enclose ions in square brackets. On your answer sheet, state the number of valence electrons in each compound. (a) NaCN (b) CH 3 Br (c) Ca(OCl) 2arrow_forwardCyanogen (CN)2 is known as pseodohalogen because it has some properties like halogens. It is composed of two CN’s joined together.(i) Draw the Lewis structure for all the possible combination for (CN)2.(ii) Calculate the formal charge and determine which one of the structures that you have drawn is most stable.(iii) For the stable structure, determine the geometry around the two central atoms.(iv) For the stable structure, draw the dipole arrows for the bonds.(v) Base on the stable structure, determine the polarity of molecule and state your reason.arrow_forwardWhich of the following compounds are likely to have covalent bonds or are likely to have ionic bonds ? (a) CF4 (b) NaF (c) CH4 (d) MgBr2arrow_forwardarrow_back_iosSEE MORE QUESTIONSarrow_forward_ios
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning